Chapter 15, Problem 15.58SP

Interpretation Introduction

Interpretation:

The percent dissociations of ${\text{HN}}_3$ should be calculated and percent dissociations of ${\text{HN}}_3$ in the presence of $\text{0}\text{.10}\text{M HCl}$ should be explained.

Concept introduction:

Equilibrium expression: The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divides by the concentrate ions of the product of reactants to the power of their coefficient.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

$\text{K}\text{=}\frac{\text{Product}\text{concentrations}}{\text{Reactant}\text{concentrations}}$

$\text{pH:}$

$\text{pH}$ is a logarithmic expression to express a solution is acidic, basic or neutral.  The $\text{pH}$ scale has values between 1 and 14 and on which 7 is neutral, below 7 values are more acidic in nature and above 7 values are more basic in nature.

$\text{pH}\text{=}{\text{-log}}_{\text{10}}{\text{[H}}^{\text{+}}\text{]}$

Percent dissociations:

The percent ratio of concentration of dissociated ions to initial concentration to gives the percent dissociations.

$\text{\%}\text{=}\frac{\text{Dissociated}\text{concentration}}{\text{Initial}\text{concentration}}\text{×100}$